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You have a solution consisting of 0.10 M Cl– and 0.10 M CrO42–. You add 0.10 M silver nitrate dropwise to this solution. Given that the Ksp for Ag2CrO4 is 9.0 × 10–12, and that for AgCl is 1.6 × 10–10, which of the following will precipitate first?

Which of the following pairs of 0.100 mol L-1 solutions, when mixed, will produce a buffer solution?

The sodium salt, NaA, of a weak acid is dissolved in water; no other substance is added. Which of these statements (to a close approximation) is true?

Which of the following is true for a buffered solution?

A solution is 2.00 x 10-3 M Ba(NO3)2 and 0.0500 M KF.  Given that the Ksp of barium fluoride is 1.5 x 10-6,

Which of the following leads to the formation of a precipitate?

Which of the following is the equilibrium constant expression for the dissociation of the weak acid HOCl?

Please Circle A2 on your Free Response Sheet You titrate 40.0 mL of 0.39 M unknown Acid with 0.37 M NaOH.  The pH at half-equivalence was 4.05.  Use the graph paper provided to draw the titration curve for this unknown acid.    Make sure your graph is properly labeled and contains the following (show your work for each calculation): initial pH mL to half equivalence and pH at half-equivalence mL to equivalence and pH at equivalence pH 10 mL after equivalence

Which of the following solutions will be the best buffer at a pH of 9.26? (Ka for HC2H3O2 is 1.8 × 10–5, Kb for NH3 is 1.8 × 10–5).

Assume an indicator works best when the equivalence point of a titration comes in the middle of the indicator range. Which indicator would be best for the following titration?0.100 M HOCl (Ka = 3.5 × 10–8) + 0.100 M NaOH